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Asked by Pavan Last Modified
Answer In the liquid state, hydrogen fluoride (HF) molecules experience two primary types of intermolecular forces:
Hydrogen Bonding: The hydrogen atom in HF is covalently bonded to the fluorine atom. Due to the high electronegativity of fluorine, the hydrogen atom in HF has a partial positive charge (δ+), while the fluorine atom has a partial negative charge (δ-). This creates a strong dipole-dipole interaction between neighboring HF molecules, known as hydrogen bonding. In hydrogen bonding, the δ+ hydrogen atom of one HF molecule is attracted to the δ- fluorine atom of another HF molecule, resulting in a relatively strong intermolecular force.
London Dispersion Forces (Van der Waals Forces): In addition to hydrogen bonding, HF molecules also experience London dispersion forces, which are also known as van der Waals forces. These forces arise from temporary fluctuations in the electron distribution within molecules, leading to temporary dipoles. These temporary dipoles induce similar temporary dipoles in neighboring molecules, resulting in an attractve force between the molecules. While London dispersion forces are generally weaker than hydrogen bonding, they still contribute to the overall intermolecular interactions between HF molecules in the liquid state.
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